Answer:
Strong acids are assumed 100% dissociated in water- True
As a solution becomes more basic, the pOH of the solution increases- false
The conjugate base of a weak acid is a strong base- true
The Ka equilibrium constant always refers to the reaction of an acid with water to produce the conjugate base of the acid and the hydronium ion- True
As the Kb value for a base increases, base strength increases- true
The weaker the acid, the stronger the conjugate base- true
Explanation:
An acid is regarded as a strong acid if it attains 100% or complete dissociation in water.
The pOH decreases as a solution becomes more basic (as OH^- concentration increases).
Ka refers to the dissociation of an acid HA into H3O^+ and A^-.
The greater the base dissociation constant, the greater the base strength.
The weaker an acid is, the stronger , its conjugate base will be.
I think its A. because there are nuclear fusion and nuclear fission
Answer:
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Explanation:
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Answer:
[H⁺] = 1.58x10⁻⁶M; [OH⁻] = 6.31x10⁻⁹M.
pH = 8.23; pOH = 5.77
Explanation:
pH is defined as <em>-log [H⁺]</em> and also you have <em>14 = pH + pOH </em>
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Thus, for a solution of pH = 5.80.
5.80 = -log [H⁺] → [H⁺] = 10^-(5.80) = 1.58x10⁻⁶M
pOH = 14-5.80 = 8.20 → [OH⁻] = 10^-(8.20) = 6.31x10⁻⁹M
Thus, for a solution of [H⁺] = 5.90x10⁻⁹M and pH = -log 5.90x10⁻⁹M = 8.23
And pOH = 14-8.23 = 5.77
Explanation:
molecular collisions. reactant particles must collide with one another before any reaction can occur.
activation energy. colliding particles must possess a certain minimum total amount of energy if the collision is result in reaction.
